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sweet [91]
2 years ago
6

There are islands in the ocean that are growing larger. The Hawaiian Islands are good examples of this. The reason that the isla

nds were formed and are still growing is A) they were produced by drought. B) they were produced by volcanoes. C) they were produced by hurricanes. D) they were produced by earthquakes.
Chemistry
1 answer:
Inessa [10]2 years ago
5 0
My guess would be "B) they were produced by volcanoes" because hawaii has a bunch of volcanoes and volcanoes can produce extra land. While the other answers wouldn't make sense. Definitely B.
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Which of the following types of radiation can be shielded by piece of paper or fabric
Keith_Richards [23]
There are 3 major types of radiation. The Alpha, Beta and Gamma radiation. It is the Alpha radiation that can be stopped by a piece of paper or fabric. Beta on the other hand can be stopped by plastic or a thin sheet of metal and Gamma by a piece of aluminum foil or lead. 
8 0
2 years ago
You find small pieces of ice instead of ice cubes in the freezer. State how this is possible.
Nat2105 [25]
Well, if u had a spilled liquid in there (we'll simply go with water) and you had the freezer at a cold temperature it would change (like,icycles on trees when it's snowing)
4 0
3 years ago
Why would there be a concern with glaciers melting because of global warming?
vaieri [72.5K]
The correct answer is C. because it could lead to an increase in ocean levels
5 0
2 years ago
How much thermal energy is added to 10.0 g of ice at −20.0°C to convert it to water vapor at 120.0°C?
Sonbull [250]

Answer:

7479 cal.

31262.2 joules

Explanation:

This is a calorimetry problem where water in its three states changes from ice to vapor.

We must use, the calorimetry formula and the formula for latent heat.

Q = m . C . ΔT

Q = Clat . m

First of all, let's determine the heat for ice, before it melts.

10 g . 0.5 cal/g°C ( 0° - (-20°C) = 100 cal

Now, the ice has melted.

Q = Clat heat of fusion . 10 g

Q = 79.7 cal/g . 10 g → 797 cal

We have water  at 0°, so this water has to receive heat until it becomes vapor. Let's determine that heat.

Q = m . C . ΔT

Q = 10 g . 1 cal/g°C (100°C - 0°C) → 1000 cal

Water is ready now, to become vapor so let's determine the heat.

Q = Clat heat of vaporization . m

Q = 539.4 cal/g . 10 g → 5394 cal

Finally we have vapor water, so let's determine the heat gained when this vapor changes the T° from 100°C to 120°

Q = m . C . ΔT

Q = 10 g . 0.470 cal/g°C . (120°C - 100°C) → 94 cal

Now, we have to sum all the heat that was added in all the process.

100 cal + 797 cal + 1000 cal + 5394 cal + 94 cal =7479 cal.

We can convert this unit to joules, which is more acceptable for energy terms.

1 cal is 4.18 Joules.

Then, 7479 cal are (7479 . 4.18) = 31262.2 joules

6 0
3 years ago
Thermal energy always moves from a greater energy level to a lesser energy level
Nookie1986 [14]

Answer:

\fbox{Law -Based \: on \: laws \: of \: thermodynamic}

Explanation:

At constant pressure Thermal energy always moves from a greater energy level to a lesser energy level, laws of thermodynamics prove that.

Nature always likes to attain equilibrium either it's movement of heat energy or flow of water from higher region to lower region. The first and second law of thermodynamics are profe of that, the first law says that the total energy of universe is Constant. Energy can not be destroyed it always changes from one form to another, by work and heat. The second law explains why thermal energy moves from a greater energy level to a lesser energy level, it deals with the change in entropy of a system and surrounding and states heat flows from hot environment to cold environment.

<em><u>Thanks for joining brainly community!</u></em>

6 0
2 years ago
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